Trends in the periodic table
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The document summarizes trends in properties of elements as you move through the periodic table, including atomic radius, ionic radii, ionization energy, electron affinity, and electronegativity. It explains that atomic radius increases down a family due to increasing energy levels, while decreasing left to right due to more protons. Ionic radii decrease when gaining electrons and increase when losing electrons. Ionization energy increases when removing electrons due to stronger nuclear attraction and decreases down a family and increases left to right. Electron affinity and electronegativity both increase left to right and decrease top to bottom.
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2. Atomic size decreases as you move across a period due to increased nuclear charge, and increases as you move down a group due to additional electron shells providing more shielding.
3. Ions form when atoms gain or lose electrons. Cations form when atoms lose electrons, becoming positively charged. Anions form when atoms gain electrons, becoming negatively charged.
4. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom.
5. Ionization energy increases
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1. This document provides an overview of trends in the periodic table, including atomic size, ionization energy, electronegativity, and metallic/non-metallic character. It explains that these properties trend both across periods, from left to right as atomic number increases, and down groups as additional shells are filled.
2. Specifically, it notes that atomic size decreases across periods as nuclear charge increases, while increasing down groups as additional shells are added. Ionization energy and electronegativity both increase from left to right as nuclear charge increases, while decreasing down groups as electrons are farther from the nucleus. Metallic character increases down groups and decreases across periods.
3. The document aims to explain these
periodic table trends
The Periodic Table and Periodic Law SECTION 3 Periodic Trends
ionization energy
atomic radius
electronegativity
Periodic trends lecture notes a.k
The document discusses several periodic trends, including how atomic radius, ionic radius, ionization energy, and electronegativity change across periods and down groups in the periodic table.
[1] Atomic radius decreases and ionization energy increases when moving across a period as nuclear charge increases, while trends are opposite when moving down a group as additional energy levels are added.
[2] Ionic radius follows the same trends as atomic radius, decreasing across periods and increasing down groups.
[3] Electronegativity also decreases down groups as the distance between nucleus and electrons increases, but increases across periods as nuclear charge rises.
Lecture 6.3- Periodic Trends (Honors)
This document contains information about periodic trends in atomic properties such as size, ionization energy, and electronegativity. It explains that atomic size generally increases down a group and decreases left to right across a period as the number of protons increases. Ionization energy decreases down a group as outer electrons are more easily removed, and increases left to right as atoms get smaller. Electronegativity also increases left to right as atoms get smaller, allowing them to better attract electrons.
Periodic properties of the elements
periodic properties of the elements for class 11th and 12th science students..go and copy all the stuff
Periodic Trends
1. The document discusses several periodic trends including atomic radius, ionization energy, and electronegativity. It explains that atomic radius decreases left to right within a period and increases down a group. Ionization energy generally increases left to right within a period and decreases down a group. Electronegativity increases left to right within a period and decreases down a group.
2. The document also discusses ionic radius trends, explaining that the size of positive ions decreases left to right within a period while the size of negative ions increases. Ionic radius increases down a group for both positive and negative ions.
3. The octet rule is mentioned as determining what types of ions atoms will form in order to acquire
Properties of periodic table by Saliha Rais
The presentation "Properties of Periodic Table" is prepared for grade IX students. The slide show includes a brief description on the properties of elements in the periodic table, that shifts periodically, hence explaining the concept of periodicity. the main topics include Atomic Radii, Ionization energy, Electron affinity and Electronegativity.
Periodicity 1
Atomic radius and ionic radius decrease moving across a period but increase moving down a group as more electron shells are added. Ionization energy increases across a period as more protons attract electrons, making them harder to remove, but decreases down a group as electrons are farther from the nucleus. Metallic character decreases across a period as more protons attract electrons closer, but increases down a group.
Regents Chemistry - Atomic Trends
Regents Chemistry - Atomic Trends
Includes information about atomic radius, ionization energy, electronegativity and electron affinity. Included are comprehension questions as well.
Note that there is an Atomic Trends table on the Reference Tables for Chemistry Regents that is used for the questions.
periodic table and periodicity
Grade 10 CAPS-aligned Periodicity notes. Looks at ionisation energy, electron affinity, electronegativity and atomic radii.
Ionic Trends
The document discusses ionic trends in atomic radius, ionization energy, and electronegativity across the periodic table. It explains that atomic radius generally decreases from left to right as more protons are added to the nucleus, attracting the electrons closer. Ionization energy decreases from right to left as the right side has more full valence shells, making them less likely to lose electrons. Electronegativity increases from left to right and decreases down groups as the distance from the valence electrons to the nucleus changes.
Ionization potential and electron affinity
1) The document discusses trends in ionization potential and electron affinity across the periodic table. Ionization potential generally increases from left to right in a period as nuclear charge increases and atomic radius decreases. It also decreases down a group as atomic size increases.
2) Electron affinity generally increases from left to right as nuclear charge increases but decreases down a group as atomic size increases. Elements in the lower left of the periodic table tend to have lower ionization potentials and are more metallic.
3) Factors that influence ionization potential and electron affinity include effective nuclear charge, atomic size, shielding effects, and stability of electron configurations.
PT IRE
The document discusses periodic trends in atomic properties including atomic radius, ionization energy, and electronegativity. It explains that as you move down a group in the periodic table, atomic radius increases while ionization energy and electronegativity decrease due to increased electron shielding. However, as you move across a period, atomic radius decreases while ionization energy and electronegativity increase due to the stronger effective nuclear charge pulling electrons in more tightly.
Electron Affinity And Ionization Energy
The document discusses energy gaps between electron shells in atoms. Electrons occupy discrete energy levels organized into shells. The energy required to excite an electron to a higher shell is equal to the energy released as light when the electron returns to a lower shell. Different elements emit different colors of light corresponding to their unique electron shell energy gaps. Fireworks emit various colors from metal salts as the metals' electrons move between shells and release energy as light.
Periodic trends
The document discusses periodic trends in elemental properties, including atomic radius, ionization energy, electron affinity, electronegativity, and reactivity. It explains that Dmitri Mendeleev was the first to organize elements into a periodic table based on their properties and predicted undiscovered elements. The trends are due to changes in atomic structure and the effective nuclear charge as protons and electrons are added. Atomic radius generally decreases left to right and increases top to bottom. Ionization energy and electronegativity increase as you move up and to the left on the periodic table.
Basic Interactions Between X Rays and Matter
X-rays can interact with matter through various processes. The most common interactions in diagnostic radiology are the photoelectric effect, Compton scattering, and coherent scattering. In the photoelectric effect, an incoming x-ray photon ejects an inner shell electron, leaving behind characteristic radiation. Compton scattering involves x-ray photon deflection by a free electron, producing scatter radiation. Coherent scattering changes a photon's direction but not its energy. These interactions have different probabilities depending on the photon energy and the electron binding energy.
Periodic Trends
1) Periodic trends refer to how properties of elements change regularly when arranged in order of increasing atomic number. These properties include atomic radius, ionization energy, and electronegativity.
2) Atomic radius generally increases moving left to right and decreases moving up a group. Ionization energy follows the opposite trend, increasing up and right as atomic radius decreases. Electronegativity also increases up and right.
3) The trends are due to changes in the number of protons, electrons, and shielding of core electrons that affect the attraction between electrons and the nucleus across the periodic table.
Periodic Trends
1) Periodic trends refer to how properties of elements change regularly when arranged in order of increasing atomic number. These properties include atomic radius, ionization energy, and electronegativity.
2) Atomic radius generally increases moving left to right and decreases moving up a group. Ionization energy follows the opposite trend, increasing up and right as atomic radius decreases. Electronegativity also increases up and right.
3) The trends are due to changes in the number of protons, electrons, and shielding of core electrons that affect the attraction between electrons and the nucleus across the periodic table.
Ch07 outline
The document summarizes periodic trends in atomic and ionic sizes, ionization energies, and electron affinities. It discusses how effective nuclear charge affects these properties and how trends are rationalized. It also describes the characteristic properties of representative elements in each group of the periodic table.
AP Chemistry Chapter 7 Outline
The document summarizes periodic trends in atomic and ionic sizes, ionization energies, and electron affinities. It discusses how effective nuclear charge affects these properties and how trends are rationalized. It also describes the characteristic properties of representative elements in each group of the periodic table.
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Molecular geometry
The document discusses molecular geometry and how the shapes of molecules can be predicted using the valence shell electron pair repulsion (VSEPR) model. It defines key terms like bonding pairs, lone pairs, and electron domains. It then provides examples of different molecular shapes like linear, trigonal planar, tetrahedral, and octahedral along with example molecules and diagrams.
Chemical bonding
The document discusses different types of chemical bonding:
1) Ionic bonding occurs when atoms transfer electrons to form ions that are attracted via opposite charges. Ionic compounds form crystal lattices and are hard, brittle, and have high melting points.
2) Covalent bonding occurs when atoms share electrons, forming either polar or nonpolar bonds. Covalent compounds have weaker attractions and are typically liquids, gases or network solids. They have low melting points and conduct limited electricity.
3) Valence electrons are those in the outermost shell that form bonds. The Lewis structure model represents these electrons with dots.
History periodic table
The document provides a history of the periodic table, from early classifications of elements by their properties to the modern periodic table organized by atomic number. It describes Lavoisier's initial grouping of 33 elements, Döbereiner's discovery of triads of elements with similar properties, Newlands' observation of an octave pattern in properties, and Mendeleev and Meyer's development of the first periodic tables by listing elements in order of atomic weight and accounting for unknown elements and switched positions. The modern periodic table is based on ordering by increasing atomic number according to the Periodic Law.
The periodic table
The document discusses the periodic table and its organization into groups and periods. It provides details on the properties and trends of each of the 18 groups, including metals, nonmetals, metalloids and noble gases. It also covers the lanthanide and actinide series located below the main body of the periodic table.
Quantum numbers
Erwin Schrodinger developed wave equations to describe the probabilities of electron locations in atoms, since electrons cannot be precisely located. He used sets of integers called quantum numbers to describe possible electron locations, including: 1) The principal quantum number representing the electron's energy level, 2) The azimuthal quantum number representing the subshell (s, p, d, f), and 3) The magnetic quantum number representing the number of orbitals in the subshell. The spin quantum number represents the electron's spin as either +1/2 or -1/2. Quantum numbers are used to describe electron configurations of elements.
Matter
This document discusses the different states of matter: solid, liquid, gas, and plasma. It describes the key properties of each state - solids have a definite shape and volume, liquids take the shape of their container but have a definite volume, gases have no definite shape or volume and can be compressed, and plasma is an ionized gas that makes up most visible matter in the universe. It also introduces condensates as a state of matter that occurs at low temperatures where atoms occupy the same quantum state.
Atoms subatomic particles
Atoms are made up of subatomic particles including electrons, protons, and neutrons. The mass number of an atom is the total number of protons and neutrons, while the atomic number refers specifically to the number of protons which determines the type of element and is also equal to the number of electrons. The number of neutrons can be calculated by taking the mass number and subtracting the atomic number.
Atoms
Atoms are the smallest particles that make up all matter. According to Dalton's atomic theory, all atoms of a given element are identical, while atoms of different elements have different properties and combine in fixed ratios. Chemical reactions rearrange atoms, but do not create or destroy them, as stated by the law of conservation of mass. The law of definite proportions says that samples of a compound contain the same proportions by mass, while the law of multiple proportions states that masses of an element combining with a fixed mass are in ratios of small whole numbers. Early atomic models included Thomson's "plum pudding" model and Rutherford's nuclear model, which showed that atoms have a small, dense nucleus containing most of their mass.
Properties of matter
Physical and chemical properties are distinguishing characteristics used to identify matter. Chemical properties involve changes in composition when substances react, while physical properties can be observed without reactions. There are two types of physical properties - intensive properties do not depend on amount, while extensive properties change with amount.
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Trends in the periodic table
- 1. Trends in the Periodic Table
- 3. Summary
- 8. Ionic Radii
- 9. Atomic and Ionic Radii